Please help me answer this question **Question 10:****Arrange the following in order of increasing boiling point and explain your reasoning (hint: structures shown are skeletal structures and may not show the complete picture).****Explain your answer, being sure to use the ideas of forces and energy.**Structures:- **A:** CH₃CH₂CH₂CH₃- **B:** CH₃CH₂CH₃- **C:** CH₃OH- **D:** CH₄- **E:** CH₃CH₂OH### Explanation:When arranging substances in order of increasing boiling point, consider the types of intermolecular forces present and the molecular structure. 1. **CH₄ (D):** Methane has the lowest boiling point due to its small, non-polar molecular structure, which only exhibits weak London dispersion forces.2. **CH₃CH₂CH₃ (B):** Propane has a higher boiling point than methane because it is a larger non-polar molecule with stronger London dispersion forces than methane.3. **CH₃CH₂CH₂CH₃ (A):** Butane, being a larger non-polar molecule than propane, will have even stronger London dispersion forces, resulting in a higher boiling point.4. **CH₃OH (C) and CH₃CH₂OH (E):** Both methanol and ethanol exhibit hydrogen bonding due to the hydroxyl groups, which significantly increase the boiling point. Ethanol, being the larger molecule, has stronger London dispersion forces in addition to hydrogen bonding, giving it a higher boiling point than methanol.### Order of Increasing Boiling Point:**D (CH₄) < B (CH₃CH₂CH₃) < A (CH₃CH₂CH₂CH₃) < C (CH₃OH) < E (CH₃CH₂OH)**

A question based on organic chemistry, which is to be accomplished.Answer Increasing order of boiling points D < B < E < A < C Explanation * Greater the molecular weight, the greater would be the boiling point. * The organic compound with -OH group has intermolecular H-bond (or) intermolecular force. So, it will have greater boiling point than those without -OH. The greater the intermolecular force, the greater would be the bond energy and hence it will require greater temperature to boil. * Also, greater the no.of -OH in the given molecule, the greater would be the boiling point. * Moreover, greater the vicinity of two -OH groups, the greater would be the intermolecular H-bonding and hence the greater would be the boiling point. # The structure D has no -OH group, hence its boiling point would be the least. Practically methane exists in gaseous state at STP. # The structure B has greater molecular weight than the structure D. Hence, it has greater boiling point than D. # The structure E has 1 -OH group, that creates intermolecular H-bonding. # The structure A has 1- OH group and has greater molecular weight than the structure E. So, the boiling point of A is greater than E. # The structure C has 2 -OH groups that creates scope for intramolecular H-bonding apart from intermolecular H-bonding. Hence, it has highest boiling point among all its competitors.